color(blue)("STP"
STP is currently 0^@"C" or "273.15 K", which are equal, though the Kelvin temperature scale is used for gas laws; and pressure is "10"^5color(white)(.)"Pascals (Pa)", but most people use "100 kPa", which is equal to 10^5color(white)(.)"Pa".
You will use the ideal gas law to answer this question. Its formula is:
PV=nRT,
where P is pressure, V is volume, n is moles, R is a gas constant, and T is temperature in Kelvins.
color(blue)("Determine moles"
You may have noticed that the equation requires moles (n), but you have been given the mass of "CO"_2". To determine moles, you multiply the given mass by the inverse of the molar mass of "CO"_2", which is "44.009 g/mol".
5.0color(red)cancel(color(black)("g CO"_2))xx(1"mol CO"_2)/(44.009color(red)cancel(color(black)("g CO"_2)))="0.1136 mol CO"_2"
color(blue)("Organize your data".
Given/Known
P="100 kPa"
n="0.1136 mol"
R="8.3145 L kPa K"^(-1) "mol"^(-1)"
https://en.wikipedia.org/wiki/Gas_constant
T="273.15 K"
Unknown: V
color(blue)("Solve for volume using the ideal gas law."
Rearrange the formula to isolate V. Insert your data into the equation and solve.
V=(nRT)/P
V=(0.1136color(red)cancel(color(black)("mol"))xx8.3145 color(white)(.)"L" color(red)cancel(color(black)("kPa")) color(red)cancel(color(black)("K"))^(-1) color(red)cancel(color(black)("mol"))^(-1)xx273.15color(red)cancel(color(black)("K")))/(100color(red)cancel(color(black)("kPa")))="2.6 L CO"_2" rounded to two significant figures due to "5.0 g"